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114114
c4
Descripción
science Mapa Mental sobre c4, creado por zoetoffee el 29/05/2013.
Sin etiquetas
science
Mapa Mental por
zoetoffee
, actualizado hace más de 1 año
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Creado por
zoetoffee
hace alrededor de 11 años
134
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Resumen del Recurso
c4
testing water purity
test 4 sulfate
add hydrocloric acid
add barium chloride solution
if whie precipitate there is
test 4 halide ions
add dilute nitric acid
add 10 drops of silver nitrat solution
if precipitate fors yes there is
elements
isotopes
different form of the same element
same number of protons
different number of nutrons
same atomic number different mass number
eg carbon 12 and carbon 14
carbon 12
6 protons
6 electrons
6 nutrons
carbon 14
6 protons
6 electrons
8 neutrons
the number of nutrons is mass - atomic number
group number of electrons in outer shell
metals
crystal structure
same properties
special bonding that is in metals
held together with metalic bonding
outer electron moves freely
this creates a sea of free electrons
high
very hard dense and shiney
strong atraction between
positive ions
delocalised electrons
high melting and boling point
large energy needed to break the metallic bonds
strenght of the metallic bond decreases as atomic radious increases
and melting point
strong
hard to break
high tensil streangth
hammered into different shapes
malleable
good conducters
the delocolised electrons carry the electrical curent
they also carry heat energy
use
sausepan
stainless steal
good heat conducter
electric wiring
copper
aeroplane
aluminium
bridge
steel
ion and ionic componds
ions
charged particals
ou have to balance the + and -
2K+
k20
the potassium ion 1+ and the oxygen 2- balance because you need 2 positive to the 2 negetive
O2-
dot and cross diagram
show what happens in ionic bonding
arrows to
electron shells
shells
2nd = 8
3rd =8
1st =2
electronic configeration
eg. 12= 2,8,2
superconducters
at low teperatures
all have some resistance
mean some eletrical energy turns to heat
if cold enough
it disdsapears
dont loose any current
the catch
you can make
powet cables with no lose
fast electronic circuites
strong electromagnets
has to be colder than -265 c
hard and expencive
transition metals
catalysts
iron
harbor process
nickel
hydrogenation
colorful
copper often blue
iron (ll) often light green
iron (lll) often orange or brown
middle of the table
have typical metallic propities
atoms
the nucleus
positive protons
netrule neutrons
the nucleus it positive
electrons
negitivly charged
the electronic shell
virtually no mass
atomic number and mass
mass top number
mass total of protons and nutron
atomic number
number of protons
bottom number
number of electrons
ionic bonding
transfering electrons
atom loses or gains an electron
forms a charged partical
ions
strongley atracted to each other
+
join together
-
one electron on a shell got to go
they like to hace a full outer shell
once they get rid thy become positivley charged
they will leapat the chance to stick to a negativ ion
nearly full shell wants an extra
gain an electron to fill the shell
become negetivly charged
eg
sodium gives up an electron
NA+
chlorine picks p an atom
CL-
forms ionic bond
giant ionic lattice
made from metals and non metals
strong chemical bonds in all ions
groups
group 1 alkali metals
oxidation
loss of electrons
the more reactive the happier to lose
cold water
produces hydrogen gas
eg sodium
they fizz
reactivity increases the lower down the group
potasium get hot enough to ignight
sodium and potasium melt
alkali forms
2 Na + 2 H2O > 2 NaOH + H2
burn with charicteristic colors
lithium =red
sodium =yellow
potassium = lilac
key facts
they all have one outer electron
low melting point
low density
very soft
they always form ionic
NEVER COVALENT
group 7 halogens
key facts
they all have 7 outer electrons
as you go down they become less reactive
melting point increase
at room tempreature
chlorine
poisonoius
dense green gas
fairley reactive
iodine
dark gray crystlline solid
bromine
poisonous
orange liquid
reduction
keenn to gain an electron
become a 1- ion
stabel electronic structure
the more reactive the happier it i to gain
gain of electrons is called reduction
form salts
react with alkli metals
makes salt called METAL HALIDES
reactions eg
2 Na + Cl2 > 2 NaCl
Sodium + Chlorine > sodium chloride
2 K + Br2 > 2 KBr
potassium + bromine > potassium bromide
displace
more reactive halogen dispalce less reactive ones
eg
Chlorine + potassium iodide > iodine+ potassium chloride
covalent bonding
sharing electrons
non metals combine to for convalent bonds
both atoms have a full outer shell
each provides one extra electron
dot and cross
overlap
simple molecular substances
covalent bods usely have simple molucal structures
eg H2O and CO2
held together with very strong covalent bonds
force between them is very weak
low boiling point
lowmelting point
at room tempreture gases and liquids
the dont conduct electricity
no free electrons
water purity
sea water
very expersive
in dry contrey r=they distill sea water
needs alot of energy
limited resorcesd
industrial coolent
homes for washing
ground water
aquifers
rocks trsp water
upto 70% of water comes from underground
ground water
eg lakes rivers reservoirs
run dry in summer
tap water
still contains in puritys
nitrate residue
fertalizer running off fields
lead compounds
from old pipes
pesicide residue
spraying to near lakes
tretment plants
filteration
wire mesh
takes out large twigs
sedimentation
iron sulphate is added
makes small particals clump together
chlorination
bubbled through to kill harmfull bacteria
thermal decomposition
hydroxide tests
copper (lll) = blue solid
iron (ll) = gray/green solid
iron (ll) = orange/brown solid
solid forms in solution
2 solution react and make a solid in the solution
called a precipitate
breaking down with heat
breaks into at leat 2 other substances
break down into metal oxide and carbon dioxide
eg. copper oxide
check for carbon dioxide = lime water
history
theories backed up
so that it can be checked for errors
so other scientists can use it to develope there own work
time line
john darlton
jj thomson
rutherford
gold foil experimenthe came up with the thery of the nuclear atom found that the plum pudding was wrong
bohr
electrons can only exist in fixed orbits
it was pretty clos to our current accepted verrsion
found the charges and mass whch showed they wernt solid spheres new thery was called the plum pudding
described them as solid spheres and said that different spheres made different elements
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